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The relationship between electric charge and the weight of deposited material on electrodes is fundamentally described by Faraday's Law of Electrolysis. This law states that the amount of chemical change (which can be quantified in terms of the weight of the substance deposited or dissolved) is directly proportional to the electric charge passed through the system.

In practical terms, this means that if you know the total charge that has flowed through the electrode, you can calculate the amount of the substance that will be deposited or consumed in the electrochemical reaction. Faraday's Law relates the chemical and physical changes in the electrochemical process to the total charge, providing a quantitative basis for predicting how much material is deposited based on the managemet of electric current.

Understanding this relationship is crucial in applications such as electroplating, battery design, and other electrochemical processes where the control of deposition and dissolution of materials at electrodes is necessary.